Arrange these compounds in order of increasing boiling...

Arrange these compounds in order of increasing boiling point. Use the boiling point values of $0^{\circ} \mathrm{C}, 35^{\circ} \mathrm{C}$ and $97^{\circ} \mathrm{C}$ (a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$ (b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}$ (c) $\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}$

Arrange these compounds in order of increasing boiling point. Use the boiling point values of $0^{\circ} \mathrm{C}, 35^{\circ} \mathrm{C}$ and $97^{\circ} \mathrm{C}$
(a) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}$
(b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}$
(c) $\quad \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}$

Key Concepts

Intermolecular Forces

Intermolecular forces play a critical role in determining boiling points. These forces, which include hydrogen bonding, dipole-dipole interactions, and London dispersion forces, must be overcome for a substance to transition from liquid to gas. The stronger these forces, the higher the boiling point of the compound.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of intermolecular interaction occurring when hydrogen is directly bonded to highly electronegative atoms like oxygen. This interaction significantly raises the boiling point of compounds capable of hydrogen bonding compared to those that only exhibit weaker forces.

Polarity

Molecular polarity refers to the uneven distribution of electron density in a molecule, leading to partial positive and negative charges. Polar molecules experience attractive dipole-dipole interactions, which enhance the intermolecular forces and contribute to higher boiling points relative to non-polar molecules.

Molecular Structure

The structure of a molecule, including its functional groups and overall geometry, influences its physical properties such as boiling point. Functional groups like hydroxyl groups can enable hydrogen bonding, while nonpolar chains predominantly exhibit weaker London dispersion forces, thereby affecting the energy required for phase transition.

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